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The low solubility of LiF in water is due to its
- a)high lattice enthalpy.
- b)small hydration enthalpy.
- c)small lattice enthalpy.
- d)high hydration enthalpy.
Correct answer is option 'A'. Can you explain this answer?
Most Upvoted Answer
The low solubility of LiF in water is due to itsa)high lattice enthal...
The solubility of a salt in water depends upon two factors
(a) Lattice enthalpy
(b) Hydration enthalpy
If the hydration enthalpy is higher than the lattice enthalpy, then the salt is soluble in water. However, if the hydration enthalpy is less than lattice enthalpy, the salt is insoluble in water.
LiF is almost insoluble in water due to its high lattice enthalpy. Both the ions in LiF are small in the size and are heavily hydrated. However, because of the high charge density on both the ions, the lattice enthalpy is also very high. So, in the case of LiF, the lattice enthalpy exceeds the hydration enthalpy because of which it is almost insoluble in water.
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The low solubility of LiF in water is due to itsa)high lattice enthal...
Understanding the Solubility of LiF in Water
The solubility of lithium fluoride (LiF) in water is primarily influenced by its high lattice enthalpy. Let's delve into the details:
High Lattice Enthalpy
- Definition: Lattice enthalpy is the energy released when gaseous ions come together to form a solid ionic compound.
- Strong Ionic Bonding: LiF has a very high lattice enthalpy due to the strong electrostatic forces between the lithium ions (Li+) and fluoride ions (F-). This strong ionic bond makes it energetically unfavorable for the solid to dissolve in water.
Comparison with Hydration Enthalpy
- Hydration Enthalpy: This is the energy change when ions are surrounded by water molecules.
- Low Hydration for LiF: Although LiF does have a small hydration enthalpy, it is not sufficient to overcome the high lattice enthalpy. Thus, the energy required to break the ionic bonds in solid LiF far exceeds the energy gained from hydration.
Conclusion
- Overall Solubility: The combination of high lattice enthalpy and comparatively lower hydration enthalpy leads to the conclusion that LiF has low solubility in water.
- Implication: In practical terms, this means that when LiF is added to water, it does not dissolve significantly, highlighting the importance of lattice enthalpy in solubility.
In summary, the high lattice enthalpy of LiF is the primary reason for its low solubility in water, making it a noteworthy example in studies of ionic compounds and their behavior in solvents.
The solubility of lithium fluoride (LiF) in water is primarily influenced by its high lattice enthalpy. Let's delve into the details:
High Lattice Enthalpy
- Definition: Lattice enthalpy is the energy released when gaseous ions come together to form a solid ionic compound.
- Strong Ionic Bonding: LiF has a very high lattice enthalpy due to the strong electrostatic forces between the lithium ions (Li+) and fluoride ions (F-). This strong ionic bond makes it energetically unfavorable for the solid to dissolve in water.
Comparison with Hydration Enthalpy
- Hydration Enthalpy: This is the energy change when ions are surrounded by water molecules.
- Low Hydration for LiF: Although LiF does have a small hydration enthalpy, it is not sufficient to overcome the high lattice enthalpy. Thus, the energy required to break the ionic bonds in solid LiF far exceeds the energy gained from hydration.
Conclusion
- Overall Solubility: The combination of high lattice enthalpy and comparatively lower hydration enthalpy leads to the conclusion that LiF has low solubility in water.
- Implication: In practical terms, this means that when LiF is added to water, it does not dissolve significantly, highlighting the importance of lattice enthalpy in solubility.
In summary, the high lattice enthalpy of LiF is the primary reason for its low solubility in water, making it a noteworthy example in studies of ionic compounds and their behavior in solvents.
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The low solubility of LiF in water is due to itsa)high lattice enthalpy.b)small hydration enthalpy.c)small lattice enthalpy.d)high hydration enthalpy.Correct answer is option 'A'. Can you explain this answer? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The low solubility of LiF in water is due to itsa)high lattice enthalpy.b)small hydration enthalpy.c)small lattice enthalpy.d)high hydration enthalpy.Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The low solubility of LiF in water is due to itsa)high lattice enthalpy.b)small hydration enthalpy.c)small lattice enthalpy.d)high hydration enthalpy.Correct answer is option 'A'. Can you explain this answer?.
The low solubility of LiF in water is due to itsa)high lattice enthalpy.b)small hydration enthalpy.c)small lattice enthalpy.d)high hydration enthalpy.Correct answer is option 'A'. Can you explain this answer? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The low solubility of LiF in water is due to itsa)high lattice enthalpy.b)small hydration enthalpy.c)small lattice enthalpy.d)high hydration enthalpy.Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The low solubility of LiF in water is due to itsa)high lattice enthalpy.b)small hydration enthalpy.c)small lattice enthalpy.d)high hydration enthalpy.Correct answer is option 'A'. Can you explain this answer?.
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